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Which of the following species has the highest bond energy?
(A)- O22
(B)- O2+
(C)- O2
(D)- O2

Answer
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Hint: Bond energy is the energy required to break one mole of a bond to separate the bonded atoms in the gaseous state. It can also be defined as the amount of energy released when one mole of a particular bond is formed between gaseous atoms. Bond energy of a bond is directly proportional to the multiplicity of the bond, i.e. its bond order.

Complete step by step answer:
Bond order tells us the number of covalent bonds present in a molecule. We know that bond energy increases with the bond order. So the molecule having the highest bond order will have the highest bond energy.
 Thus, let us calculate the bond order in the given species.
Bond order is mathematically calculated as half the difference between the number of electrons in the bonding and number of electrons in the antibonding orbitals. If Nb and Na are the number of bonding and antibonding electrons, respectively, then bond order is given as
     Bond order=12(NbNa)

Electronic configuration of oxygen, O (Z=8): 1s22s22px22py12pz1.
Electronic configuration of oxygen molecule, O2 :
     σ1s2σ1s2σ2s2σ2s2σ2pz2π2px2π2py2π2px1π2py1

Bond order of peroxide ion O22
Oxygen molecule (O2) has 16 electrons. It gains 2 electrons to form O22 ion. The two electrons gained will be added into half filled π2px1 and π2py1 such that the electronic configuration of O22 is σ1s2σ1s2σ2s2σ2s2σ2pz2π2px2π2py2π2px2π2py2.

Now, the total number of electrons in bonding molecular orbitals, Nb = 10
Total number of electrons in the antibonding molecular orbitals, Na = 8
Therefore, the bond order of O22 will be
Bond order = 12(NaNb)
Bond order = 12(108)=1

Bond order of O2+ ion.
One electron is lost from π2px1 (or π2py1) molecular orbital of O2 molecule to form O2+ ion. Since, one electron is lost from antibonding molecular orbital, the electronic configuration of O2+ ion becomes
     σ1s2σ1s2σ2s2σ2s2σ2pz2π2px2π2py2π2px1π2py0 .
Total number of electrons in bonding molecular orbitals, Nb = 10
Number of electrons in the antibonding molecular orbitals, Na = 5
Therefore, bond order = 12(105)=2.5=212

Bond order of O2 superoxide ion
O2 molecule gains one electron into π2px1 (or π2py1) to form O2 ion. Now the electronic configuration of O2 is σ1s2σ1s2σ2s2σ2s2σ2pz2π2px2π2py2π2px2π2py1.

Number of bonding electrons, Na = 10
Number of antibonding electrons, Nb = 7
Therefore, bond order of O2 = 12(107)=1.5=112

Bond order of oxygen molecule, O2
We know that electronic configuration of O2 molecule is given as
     σ1s2σ1s2σ2s2σ2s2σ2pz2π2px2π2py2π2px1π2py1
O2 molecule has 10 electrons in bonding molecular orbitals and 6 electrons in antibonding molecular orbitals, thus its bond is calculated to be
     12(NbNa)=12(106)=2
Therefore, the bond order of the given species follows the order, i.e. O2+>O2>O2>O22.

Since, bond energy increases with the increase of bond order. So, the bond energy of the species also follows the same order as the bond order, i.e.
     O2+>O2>O2>O22
Thus, O2+ has the highest bond order, and hence the highest bond energy.

So, the correct answer is “Option B”.

Note: Greater the bond order, higher the bond energy and hence, greater is the stability. Note that the energy of σ2pz is less than that of π2px and π2py molecular orbitals and energy of both the π-orbitals, π2px and π2py is the same in case of O2, i.e. σ2pz<π2px=π2py.
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